1. Intro a. Least common state of matter in universe b. Can only exist within a relatively narrow range of temps 2. Properties a. Definite volume and takes shape of container b. Particles in constant motion c. Particles closer than gas particles

d. Particles more ordered than w/gases e. Fluid – substance that can flow and take shape of its container f. Relatively High Density 1) More dense than gas 2) Less dense than solid (typically) g. Can compress slightly – not as much as gas h. Pressure equally distributed in all directions

i. Can diffuse 1) Caused by browning movement 2) High to low concentration 3) Warmer liquids diffuse faster Diffusion Rate Lab

j. Surface Tension 1) Force that pulls adjacent particles together decreasing surface area (typically sphere) 2) Caused by cohesion Fiery bubbles

3) Capillary action – attraction of liquid to solid a) Adhesion b) Goes up until weight of liquid = gravitational force c) Causes meniscus, helps bring water from roots to leaves Find different tubes to do this with

4) Vaporization – liquid to gas a) Evaporation i. slow process ii. Particles have higher-than- ave energies which allows them to overcome intermolecular forces b) Boiling – fast process

5) Formation of Solids a) Cooling (removing heat) lowers energy of particles b) Particles become attracted to each other c) Form an orderly arrangement of particles d) Freezing

1. Properties a. Particles very closely packed b. Intermolecular forces very strong c. Definite volume and shape d. 2 types 1)Crystalline (pg 369) a)Most solids b)Have crystals (geometric pattern)

2) Amorphous – particles arranged randomly e. Definite Melting point 1) Melting – solid to liquid 2) Melting pt – temp at which melting takes place

f. High density – most dense of all states of matter (typically) g. Can’t be compressed h. Low rate of diffusion 2. Crystalline Solids a. Can be single crystal or groups of crystals b. Crystal structure – 3D arrangement of particles

c. Binding Forces in Crystals (pg 370) 1) Ionic Crystals a) Hard and brittle b) High melting points 2) Covalent network crystals a) Large number of molecules in a network b) VERY hard and brittle c) non/semiconductors d) Diamonds

3) Metallic crystals a) Metal atoms surrounded by a sea of valence electrons b) B/c of val. Ele they are very good conductors 4) Covalent molecular crystals a) Covalently bonded molecules b) Low melting pts

3. Amorphous Solids a. No natural or regular shape b. Hold shape for long time c. Some can flow (very slowly)

1. Equilibrium a. Two things change at equal rates b. Changes of sta te 1)Melting 2)Freezing 3)Vaporization 4)Condensation 5)Deposition 6)Sublimation

c. Things like to be in equilibrium d. If a system is stressed it will regain equilibrium e. Stress – concentration, pressure, or temperature

f. How it works (temp) 1) Increase temp 2) Causes more to evaporate 3) This causes more vapor 4) More vapor = more can condense 5) Equilibrium is reached

g. How it works (concentration) 1) Volume is increased 2) causes surface area to increase 3) This means more evaporates 4) More can condense 5) equilibrium is reached

2. Equilibrium Vapor Pressure of Liquid a. Volatile liquids – liquids that evaporate easily (ether), weak forces b. Nonvolatile liquids – evaporate slowly, strong intermolecular forces c. Depends on only temperature Demo pg 377

3. Boiling a. Liquid to vapor b. Happens when vapor pressure of liquid = atmospheric pressure c. Boiling pt – temp when equilibrium vapor pressure = atmospheric pressure

 How does boiling pt relate to cooking on a mountain?

1) All heat goes to evaporate liquid 2) Temperature doesn’t change as long as pressure is constant d. Energy is used to overcome attractive forces 1) Stronger forces = higher boiling pts 2) Energy stored as PE

4. Freezing and Melting a. Freezing pt – temp where solid and liquid are at equilibrium b. Melting pt 1) Temp where solid becomes liquid 2) Occurs at constant temperature Demo pg 380

c. Sublimation and Deposition 1) Sub – solid directly to gas a) CO 2 b) Iodine 2) Dep – gas directly to solid

5. Phase Diagrams a. Graph of pressure vs. temp and the state of matter

b. Triple pt – pt where solid, liquid, and gas can coexist at same time c. Critical temp – temperature where substance can’t exist as a liquid no matter what the pressure (pg 381) d. Critical pressure – Lowest pressure where substance can exist a liquid at the critical temp e. Critical pt – where critical temp and pressure meet

1. Importance a. Cover 75% of earth’s surface b. Living things are 70-90% water c. Chemical reactions need water d. Frequently a reactant or product

2. Structure of Water a. Made of hydrogen and oxygen b. Bonded by polar covalent bonds c. Molecule is bent d. Angle is 105 ◦ e. Molecules held together by H bonding

3. Physical Properties of Water a. At room temp 1) Transparent 2) Odorless 3) Tasteless 4) Almost colorless

b. Boils at 100 ◦ and freezes at 0 ◦ c. Boiling pt is high compared to most liquids